The equilibrium constant (K) of the reaction below is K = 2.5 x 10-3, with initial concentrations as follows: [H₂] = 1.0 x 10-2 M, [N₂] = 4.0 M, and [NH3] = 1.0 x 10° 4 M. N2(g) + 3 H₂(g) →→→ 2 NH3(g) If the concentration of the reactant H₂ was increased from 1.0 x 10-2 M to 2.5 x 10- 1M, then the reaction quotient (Q) ip notation] [Report your answer in scientific towards the The equilibrium position would shift [left/right/or remain unchanged]. A/

The equilibrium constant (K) of the reaction below is K = 2.5 x 10-3, with initial concentrations as follows: [H₂] = 1.0 x 10-2 M, [N₂] = 4.0 M, and [NH3] = 1.0 x 10° 4 M. N2(g) + 3 H₂(g) →→→ 2 NH3(g) If the concentration of the reactant H₂ was increased from 1.0 x 10-2 M to 2.5 x 10- 1M, then the reaction quotient (Q) ip notation] [Report your answer in scientific towards the The equilibrium position would shift [left/right/or remain unchanged]. A/

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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